Question

Calculate the pressure exerted by 22 g of carbon dioxide in $0.5d{m}^3$at 300 K using:

(a) Ideal gas law and
(b) Van der Waals equation

[Given: $a=360kPad{m}^{6}mo{l}^{-2}$ and $b=40c{m}^{3}mo{l}^{-1}$]

• A. (a) 12 atm (b) 11.40 atm
• B. (a) 24 atm (b) 21.40 atm
• C. (a) 48 atm (b) 42.80 atm
• D. (a) 24.63 atm (b) 22.1 atm
  

Answer 1

The correct option is D (a) 24.63 atm (b) 22.1 atm

(a) By using the ideal gas law

$P=\frac{WRT}{MV}=\frac{22\times 0.0821\times 300}{44\times 0.5}=24.63atm$

(b) By using Van der Waals equation

$P=\frac{nRT}{(V-nb)}-\frac{a{n}^2}{V^2}=\frac{0.5\times 0.0821\times 300}{0.5-(0.5\times 40\times {10}^{-3})}-\frac{360\times {0.5}^2}{101.321\times {0.5}^2}=25.66-3.55=22.1atm$

Hence, the correct answer is option $\text{D}$.